Chapter 7

Question 1

Wavelength (λ)

Answer 1

Distance between two successive peaks or troughs

Question 2

Frequency (v)

Answer 2

Number of waves per second that pass a given point in space

Question 3

wave of light eq

Answer 3

c=vλ

Question 4

Amplitude

Answer 4

Maximum and minimum height
* Intensity of wave, or brightness
* Varies with time as travels through space

Question 5

Nodes

Answer 5

Points of zero amplitude
* Place where wave goes through axis
* Distance between nodes is constant

Question 6

Rank The lights on the EMS from shortest to longest wavelength, highest to lowest frequency.

Answer 6

Gamma, X-ray, UV, Visible, (VIBGYOR) Infrared, Microwave, Radio wave

Question 7

Which wavelength has the highest energy with the shortest wave

Answer 7

Gamma

Question 8

Which wavelength has the lowest energy and longest wave

Answer 8

radiowave

Question 9

What lightwaves can humans see

Answer 9

400-700 nm

Question 10

energy of a photon equation

Answer 10

E=hv, where h is plancks constant,v is frequency

Question 11

KE of ejected electron

Answer 11

KE=hv-BE where BE is binding energy

Question 12

energy of a mole of photons eq

Answer 12

E=nhv where n=Na=Avogadro constant, h=Planck constant, v=frequency

Question 13

Allowed values of quantum number n

Answer 13

1,2,3,4,5…etc

Question 14

Allowed values of quantum number l

Answer 14

n-1, up to zero

Question 15

allowed values for magnetic quantum number

Answer 15

-l to 0 to +l

Question 16

allowed values for spin quantum number

Answer 16

+- 0.5

Question 17

Pauli exclusion principle

Answer 17

electrons must be spin paired, you cannot have two up/two down

Question 18

Properties of electrons in the same orbital

Answer 18

-diamagnetic (spin paired)
-not attracted to magnetic field
-magnetic effects cancel out

Question 19

Properties of electrons in different orbitals with same spin

Answer 19

-paramagnetic (spin paired)
-attracted to magnetic field
-magnetic effects get stronger

Question 20

Aufbau Principle

Answer 20

Lowest energy orbitals must be filled first

Question 21

Hund’s rule

Answer 21

when filling subshells, put one e- in each subshell before spin pairing

Question 22

Valence shell configuration

Answer 22

elcectron configuration of only the outermost shell for an element

Question 23

Copper electron configuration (exception to the rule)

Answer 23

[Ar]3d10,4s1

Question 24

Chromium electron configuration (exception to the rule)

Answer 24

[Ar]3d5,4s1

Question 25

Effective Nuclear charge (Zeff)

Answer 25

Net positive charge outer electron feels Core electrons shield valence electrons from full nuclear charge

Question 26

Zeff trend

Answer 26

Increases across and down the ptables

Question 27

Zeff Formula

Answer 27

Protons-core electrons

Question 28

Atomic radius trend

Answer 28

increases down a column because n is getting bigger, decreases across a row because electrons will feel less of a pull with fewer protons

Question 29

Ionic Radii trend

Answer 29

increases down a column, decreases across a period

Question 30

IE trend

Answer 30

decreases down a column, increases across a period

Question 31

IE formula

Answer 31

A(g) → A⁺(g) + e⁻

Question 32

EA trend

Answer 32

increases down a column and across a period

Question 33

EA formula

Answer 33

X(g)+e-=X-

Question 34

Exceptions to IE rule

Answer 34

IE Be > IE B (full shell stability_ IE N > IE O (half shell stability)

Question 35

Exceptions to EA rule

Answer 35

EA Li> EA Be (filling Li 2s1 releases more energy EA C> EA N (adding an electron to C gives half shell stability) EA F > EA Ne (full shell stability)